Difference between revisions of "Zinc perchlorate"
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: ZnCO<sub>3</sub> + 2 HClO<sub>4</sub> → Zn(ClO<sub>4</sub>)<sub>2</sub> + H<sub>2</sub>O + CO<sub>2</sub> | : ZnCO<sub>3</sub> + 2 HClO<sub>4</sub> → Zn(ClO<sub>4</sub>)<sub>2</sub> + H<sub>2</sub>O + CO<sub>2</sub> | ||
| − | Do | + | Do NOT use [[zinc]] metal, as the reaction is violent! |
The resulting solution is gently heated and the product is recrystallized from the concentrated solution. | The resulting solution is gently heated and the product is recrystallized from the concentrated solution. | ||
Latest revision as of 22:29, 15 August 2022
| Names | |
|---|---|
| IUPAC name
Zinc perchlorate
| |
| Other names
Zinc(II) perhlorate
| |
| Properties | |
| ZnCl2O8 Zn(ClO4)2 (anhydrous) Zn(ClO4)2·6H2O (hexahydrate) | |
| Molar mass | 264.3 g/mol (anhydrous) 372.38 g/mol (hexahydrate) |
| Appearance | Colorless deliquescent solid |
| Odor | Odorless |
| Density | 2.26 g/cm3 (hexahydrate)[1] 2.933 g/cm3 (anhydrous) (20 °C)[2] |
| Melting point | 105–107 °C (221–225 °F; 378–380 K) (hexahydrate) 262 °C (504 °F; 535 K) (anhydrous)[4] |
| Boiling point | Decomposes |
| 50 g/100 ml (20 °C)[3] | |
| Solubility | Soluble in acetonitrile, alcohols, DMSO Slightly soluble in glacial acetic acid |
| Vapor pressure | ~0 mmHg |
| Thermochemistry | |
| Std enthalpy of
formation (ΔfH |
-2,133.77 kJ/mol[6] |
| Hazards | |
| Safety data sheet | Sigma-Aldrich (hexahydrate) |
| Related compounds | |
| Related compounds
|
Zinc chloride |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Zinc perchlorate (Zn(ClO4)2) is a hygroscopic chemical compound, that may be used as oxidizer. It is more commonly encountered as its hexahydrate form, Zn(ClO4)2·6H2O.
Contents
Properties
Chemical
Zinc perchlorate decomposes if heated to high temperatures and may explode if heated too strongly.
Physical
Zinc perchlorate is a hygroscopic colorless solid, soluble in water and low weight alcohols.
Availability
It is sold by chemical suppliers.
Preparation
Zinc perchlorate can be prepared by dissolving zinc oxide or carbonate in perchloric acid.
- ZnO + 2 HClO4 → Zn(ClO4)2 + H2O
- ZnCO3 + 2 HClO4 → Zn(ClO4)2 + H2O + CO2
Do NOT use zinc metal, as the reaction is violent!
The resulting solution is gently heated and the product is recrystallized from the concentrated solution.
Recrystallizing the salt from water yields the hexahydrate form. Anhydrous zinc perchlorate cannot be produced by heating zinc(II) perchlorate hexahydrate, since it decomposes upon heating.
One source indicates that the anhydrous form can be obtained by heating the hexahydrate with triethyl orthoformate, then drying the resulting solid under vacuum. So far this method hasn't been verified.[7]
Projects
- Source of perchlorates
- Ignite combustible materials
Handling
Safety
Zinc perchlorate is a powerful oxidizing agent. In contact with strong acids, it will ignite organic material on contact.
Storage
Zinc perchlorate should be kept in airtight bottles, away from any combustible materials.
Disposal
Can be mixed with a flammable material and ignited.
References
- ↑ West, C. D.; Zeitschrift fuer Kristallographie, Kristallgeometrie, Kristallphysik, Kristallchemie; vol. 91; (1935); p. 480 - 493
- ↑ Lyubimova, G. N.; Razumova, A. P.; Rosolovskii, V. Ya.; Russian Journal of Inorganic Chemistry (Translation of Zhurnal Neorganicheskoi Khimii); vol. 28; (1983); p. 1687 - 1688; Zhurnal Neorganicheskoi Khimii; vol. 28; (1983); p. 2975 - 2976
- ↑ Ali, Noorshida Mohd; MacLeod, Voirrey L.; Jennison, Petter; Sazanovich, Igor V.; Hunter, Christopher A.; Weinstein, Julia A.; Ward, Michael D.; Dalton Transactions; vol. 41; nb. 8; (2012); p. 2408 - 2419
- ↑ Nikitina; Rosolovskii; Russian Journal of Inorganic Chemistry; vol. 41; nb. 7; (1996); p. 1031 - 1034
- ↑ White, Mary Anne; Falk, Michael; Journal of Chemical Physics; vol. 84; nb. 6; (1986); p. 3484 - 3490
- ↑ Kon'Kova; Matyushin; Miroshnichenko; Vorob'Ev; Russian Chemical Bulletin; vol. 58; nb. 5; (2009); p. 896 - 901
- ↑ Notni, Johannes; Schenk, Stephan; Goerls, Helmar; Breitzke, Hergen; Anders, Ernst; Inorganic Chemistry; vol. 47; nb. 4; (2008); p. 1382 - 1390
